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Two solutions, A and B, each of 100 L was made by dissolving 4 g of NaOH and 9.8 g of H2SO, in water, respectively. The pH of the resultant solution obtained from mixing 40 L of solution A and 10 L of solution B is ________.
[Answer upto two decimal places]
[Answer upto two decimal places]
Correct answer is '10.60'. Can you explain this answer?
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Two solutions, A and B, each of 100 L was made by dissolving 4 g of Na...
PH is a measure of the acidity or basicity of a solution. It is defined as the negative logarithm (base 10) of the concentration of hydrogen ions (H+) in the solution. A lower pH value indicates a more acidic solution, while a higher pH value indicates a more basic solution.
In order to determine the pH of the resultant solution obtained from mixing solution A and solution B, we need to calculate the concentration of H+ ions in the final solution.
First, let's calculate the concentration of NaOH in solution A:
- Mass of NaOH = 4 g
- Molar mass of NaOH = 22.99 g/mol + 16.00 g/mol + 1.01 g/mol = 39.99 g/mol
- Number of moles of NaOH = (4 g) / (39.99 g/mol) = 0.10 mol
- Volume of solution A = 40 L
- Concentration of NaOH in solution A = (0.10 mol) / (40 L) = 0.0025 mol/L
Next, let's calculate the concentration of H2SO4 in solution B:
- Mass of H2SO4 = 9.8 g
- Molar mass of H2SO4 = 1.01 g/mol + 32.07 g/mol + (4 x 16.00 g/mol) = 98.09 g/mol
- Number of moles of H2SO4 = (9.8 g) / (98.09 g/mol) = 0.10 mol
- Volume of solution B = 10 L
- Concentration of H2SO4 in solution B = (0.10 mol) / (10 L) = 0.01 mol/L
When the two solutions are mixed, the total volume is 40 L + 10 L = 50 L. Now we can calculate the concentration of H+ ions in the final solution:
- Total moles of H+ ions = moles of NaOH + moles of H2SO4 = 0.10 mol + 0.10 mol = 0.20 mol
- Concentration of H+ ions in the final solution = (0.20 mol) / (50 L) = 0.004 mol/L
Finally, we can calculate the pH of the solution using the equation:
pH = -log[H+]
pH = -log(0.004)
pH ≈ 2 - log(4)
pH ≈ 2 - 0.60
pH ≈ 1.40
Therefore, the pH of the resultant solution obtained from mixing 40 L of solution A and 10 L of solution B is approximately 1.40.
I apologize for the incorrect answer in the question. The correct answer should be 1.40, not 10.60.
In order to determine the pH of the resultant solution obtained from mixing solution A and solution B, we need to calculate the concentration of H+ ions in the final solution.
First, let's calculate the concentration of NaOH in solution A:
- Mass of NaOH = 4 g
- Molar mass of NaOH = 22.99 g/mol + 16.00 g/mol + 1.01 g/mol = 39.99 g/mol
- Number of moles of NaOH = (4 g) / (39.99 g/mol) = 0.10 mol
- Volume of solution A = 40 L
- Concentration of NaOH in solution A = (0.10 mol) / (40 L) = 0.0025 mol/L
Next, let's calculate the concentration of H2SO4 in solution B:
- Mass of H2SO4 = 9.8 g
- Molar mass of H2SO4 = 1.01 g/mol + 32.07 g/mol + (4 x 16.00 g/mol) = 98.09 g/mol
- Number of moles of H2SO4 = (9.8 g) / (98.09 g/mol) = 0.10 mol
- Volume of solution B = 10 L
- Concentration of H2SO4 in solution B = (0.10 mol) / (10 L) = 0.01 mol/L
When the two solutions are mixed, the total volume is 40 L + 10 L = 50 L. Now we can calculate the concentration of H+ ions in the final solution:
- Total moles of H+ ions = moles of NaOH + moles of H2SO4 = 0.10 mol + 0.10 mol = 0.20 mol
- Concentration of H+ ions in the final solution = (0.20 mol) / (50 L) = 0.004 mol/L
Finally, we can calculate the pH of the solution using the equation:
pH = -log[H+]
pH = -log(0.004)
pH ≈ 2 - log(4)
pH ≈ 2 - 0.60
pH ≈ 1.40
Therefore, the pH of the resultant solution obtained from mixing 40 L of solution A and 10 L of solution B is approximately 1.40.
I apologize for the incorrect answer in the question. The correct answer should be 1.40, not 10.60.
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Two solutions, A and B, each of 100 L was made by dissolving 4 g of Na...
For given solutions, we have:
Moles of NaOH = 4/40 = 0.1
Moles of H2SO4 = 9.8/98 = 0.1
Molarity of each sample = 0.1/100 = 0.001M
Now, 40 L of NaOH solution and 10 L of H2SO4 solution are added. Thus, we get:
Total volume = 50 L
Equivalents of NaOH = 0.001 × 40 = 0.04
Equivalents of H2SO4 = 0.001 × 10 × 2 = 0.02
Thus, Eq. of NaOH left = 0.04 - 0.02 = 0.02
[OH-] = 0.02/50 = 4 × 10-4
pOH = -log[4 × 10-4]
pOH = -log4 - log10-4
pOH = -0.602 + 4 = 3.398 ≈ 3.4
Further, we know:
pH = 14 - 3.4
pH = 10.6
Moles of NaOH = 4/40 = 0.1
Moles of H2SO4 = 9.8/98 = 0.1
Molarity of each sample = 0.1/100 = 0.001M
Now, 40 L of NaOH solution and 10 L of H2SO4 solution are added. Thus, we get:
Total volume = 50 L
Equivalents of NaOH = 0.001 × 40 = 0.04
Equivalents of H2SO4 = 0.001 × 10 × 2 = 0.02
Thus, Eq. of NaOH left = 0.04 - 0.02 = 0.02
[OH-] = 0.02/50 = 4 × 10-4
pOH = -log[4 × 10-4]
pOH = -log4 - log10-4
pOH = -0.602 + 4 = 3.398 ≈ 3.4
Further, we know:
pH = 14 - 3.4
pH = 10.6
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Two solutions, A and B, each of 100 L was made by dissolving 4 g of NaOH and 9.8 g of H2SO, in water, respectively. The pH of the resultant solution obtained from mixing 40 L of solution A and 10 L of solution B is ________.[Answer upto two decimal places]Correct answer is '10.60'. Can you explain this answer?
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Two solutions, A and B, each of 100 L was made by dissolving 4 g of NaOH and 9.8 g of H2SO, in water, respectively. The pH of the resultant solution obtained from mixing 40 L of solution A and 10 L of solution B is ________.[Answer upto two decimal places]Correct answer is '10.60'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about Two solutions, A and B, each of 100 L was made by dissolving 4 g of NaOH and 9.8 g of H2SO, in water, respectively. The pH of the resultant solution obtained from mixing 40 L of solution A and 10 L of solution B is ________.[Answer upto two decimal places]Correct answer is '10.60'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Two solutions, A and B, each of 100 L was made by dissolving 4 g of NaOH and 9.8 g of H2SO, in water, respectively. The pH of the resultant solution obtained from mixing 40 L of solution A and 10 L of solution B is ________.[Answer upto two decimal places]Correct answer is '10.60'. Can you explain this answer?.
Two solutions, A and B, each of 100 L was made by dissolving 4 g of NaOH and 9.8 g of H2SO, in water, respectively. The pH of the resultant solution obtained from mixing 40 L of solution A and 10 L of solution B is ________.[Answer upto two decimal places]Correct answer is '10.60'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about Two solutions, A and B, each of 100 L was made by dissolving 4 g of NaOH and 9.8 g of H2SO, in water, respectively. The pH of the resultant solution obtained from mixing 40 L of solution A and 10 L of solution B is ________.[Answer upto two decimal places]Correct answer is '10.60'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Two solutions, A and B, each of 100 L was made by dissolving 4 g of NaOH and 9.8 g of H2SO, in water, respectively. The pH of the resultant solution obtained from mixing 40 L of solution A and 10 L of solution B is ________.[Answer upto two decimal places]Correct answer is '10.60'. Can you explain this answer?.
Solutions for Two solutions, A and B, each of 100 L was made by dissolving 4 g of NaOH and 9.8 g of H2SO, in water, respectively. The pH of the resultant solution obtained from mixing 40 L of solution A and 10 L of solution B is ________.[Answer upto two decimal places]Correct answer is '10.60'. Can you explain this answer? in English & in Hindi are available as part of our courses for JEE.
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Two solutions, A and B, each of 100 L was made by dissolving 4 g of NaOH and 9.8 g of H2SO, in water, respectively. The pH of the resultant solution obtained from mixing 40 L of solution A and 10 L of solution B is ________.[Answer upto two decimal places]Correct answer is '10.60'. Can you explain this answer?, a detailed solution for Two solutions, A and B, each of 100 L was made by dissolving 4 g of NaOH and 9.8 g of H2SO, in water, respectively. The pH of the resultant solution obtained from mixing 40 L of solution A and 10 L of solution B is ________.[Answer upto two decimal places]Correct answer is '10.60'. Can you explain this answer? has been provided alongside types of Two solutions, A and B, each of 100 L was made by dissolving 4 g of NaOH and 9.8 g of H2SO, in water, respectively. The pH of the resultant solution obtained from mixing 40 L of solution A and 10 L of solution B is ________.[Answer upto two decimal places]Correct answer is '10.60'. Can you explain this answer? theory, EduRev gives you an
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